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Magazine Chapter 3: Problem 214
In which of the following molecules, the central atom does not have \(s p^{3}\) -hybridization? \(\quad\) [C.B.S.E. (P.M.T.) 2010] (a) \(\mathrm{CH}_{4}\) \(\square\) (b) \(\mathrm{SF}_{4}\) \(\square\) (c) \(\mathrm{BF}_{4}^{-}\) \(\square\) (d) \(\mathrm{NH}_{4}^{*}\)
Short Answer
Expert verified
SF鈧� does not have sp鲁 hybridization; it has sp鲁d hybridization.
Step by step solution
01
Understanding sp鲁 Hybridization
The central atom is said to exhibit sp鲁 hybridization if it forms four equivalent hybrid orbitals, which are a combination of one s orbital and three p orbitals. This typically results in a tetrahedral geometry.
02
Examining CH鈧�
In CH鈧� (methane), the central atom is carbon, which uses its sp鲁 hybrids to form four sigma bonds with hydrogen atoms. This structure is tetrahedral, confirming sp鲁 hybridization.
03
Examining SF鈧�
SF鈧� has sulfur as the central atom, which forms four sigma bonds with fluorine and has one lone pair. This results in a 'see-saw' shape due to its sp鲁d hybridization, not sp鲁.
04
Examining BF鈧勨伝
In BF鈧勨伝, boron is the central atom and forms four equivalent B-F bonds. Boron undergoes sp鲁 hybridization here, resulting in a tetrahedral geometry.
05
Examining NH鈧勨伜
In NH鈧勨伜, nitrogen is the central atom and forms four equivalent N-H bonds, using sp鲁 hybridization. This leads to a tetrahedral shape as well.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
tetrahedral geometry
Tetrahedral geometry is a term used to describe the shape formed when a central atom is surrounded by four substituents positioned at the corners of an imaginary tetrahedron. This is a common geometric arrangement in chemistry, particularly for molecules with an atom that undergoes sp鲁 hybridization.
The tetrahedral geometry has several characteristics:
The tetrahedral geometry has several characteristics:
- Each bond angle in a tetrahedral molecule is approximately 109.5 degrees, which helps minimize the repulsion between electron pairs.
- This arrangement allows for maximum separation of the bonded pairs of electrons, which contributes to the molecule's stability.
- Molecules such as \( ext{CH}_4 \) and \( ext{BF}_4^- \) exhibit tetrahedral geometry, as each central atom forms four equivalent bonds.
hybrid orbitals
Hybrid orbitals occur when atomic orbitals mix to form new, identical orbitals suited for bonding electrons. The process allows atoms to form stronger, more stable bonds, especially notable in central atoms like carbon in methane (\( ext{CH}_4 \)).
Here's what to know about hybrid orbitals:
Here's what to know about hybrid orbitals:
- The sp鲁 hybridization involves mixing one s orbital and three p orbitals from the same energy level, leading to four hybrid orbitals.
- Each hybrid orbital has a similar shape and energy level, which allows the central atom to form equivalent bonds with surrounding atoms.
- sp鲁 hybridization leads to a tetrahedral geometry in molecules, a valuable concept in understanding molecular shapes and bond angles.
sigma bonds
Sigma bonds are the primary type of covalent bonds characterized by the head-on or end-to-end overlap of atomic orbitals. They are the single bonds formed between atoms, for example, in \( ext{CH}_4 \) and \( ext{NH}_4^+ \).
Characteristics of sigma bonds include:
Characteristics of sigma bonds include:
- They provide immense stability to molecules due to their larger degree of orbital overlap, making them stronger than pi bonds.
- Sigma bonds allow for the free rotation of bonded atoms about the bond axis, contributing to the flexibility of molecules.
- Each bond in a molecule with a tetrahedral geometry, such as \( ext{CH}_4 \), is a sigma bond arising from the overlap of sp鲁 hybrid orbitals with orbitals from surrounding atoms.
central atom
The term "central atom" refers to the atom in a molecule that is bonded to multiple other atoms. It is typically the atom with the highest bonding capacity, often playing a key role in defining the molecule's geometry.
Understanding the role of the central atom involves noting:
Understanding the role of the central atom involves noting:
- The central atom undergoes hybridization to facilitate the formation of geometrically optimal and equivalent bonds with surrounding atoms, as seen in \( ext{CH}_4 \) with carbon and \( ext{BF}_4^- \) with boron.
- When hybridized, the central atom's electron distribution significantly influences the molecule's shape and potential energy, impacting its chemical properties.
- The behavior of the central atom, like sulfur in \( ext{SF}_4 \), can lead to variations in molecular geometry, impacting the overall shape and function of the entire molecule.
